If 60 g of ethane ( C ₂ H ₆ ) is burnt in the presence of 112 g of oxygen ( O ₂ ), the mass of water produced is ______ g. (Given molar masses in g mol ⁻¹ : C = 12.0 , H = 1.0 , O = 16.0 )

Step-by-step solution

The balanced chemical equation for the combustion of ethane is: 2 C ₂ H ₆ + 7 O ₂ 4 CO ₂ + 6 H ₂ O Molar mass of ethane ( C ₂ H ₆ ) = 2 12 + 6 1 = 30 g mol ⁻¹ Moles of ethane = 60 30 = 2 mol Molar mass of oxygen ( O ₂ ) = 32 g mol ⁻¹ Moles of oxygen = 112 32 = 3.5 mol From the balanced equation, 2 mol of ethane requires 7 mol of oxygen for complete combustion. Since only 3.5 mol of oxygen is available, O ₂ is the limiting reagent. According to the stoichiometry, 7 mol of O ₂ produces 6 mol of H ₂ O . Moles of H ₂ O